To find the activation energy for the reaction it will be helpful to complete th

Question

To find the activation energy for the reaction it will be helpful to complete the following table. The dependence of the rate constant, k', for a reaction is given by Equation 4: log_10 k' = -E_a/2.30 RT + constant Find the slope of the line obtained by drawing the best straight line through the experimental points. Male the scale such that each square on the abscissa equals 0.00005 and each square on the ordinate equals 0 2. The slope of the line equals -E_a/2.30 R, where R = 8.31 joules/mole K if E_a is to be in joules per mole. Find the activation energy E_a, for the reaction. Time for color to appear (seconds) Would you expect the activation energy, E_a, for the catalyzed reaction to be greater than, less than, or equal to the activation energy for the uncatalyzed reaction? Why?

Explanation / Answer

in order to find out actvation energy

1. first you need to carry out the reaction at different temperatures.

2. At different temperatures you need to caluclate the rate of reaction, from which you need to find out reaction constant K

3. After that you need to plot the graph of Logarithm of K vs Temperature

4. Then find out the best fit line through the points and find its slope

5. Slope of graprh = activation energy/ (2.303 * R), where R= 8.314

6. activation energy = Slope og graph * 2.303 * 8.134

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